Charles' Law

Gay-Lussac's Law of Combining Volumes

In a reaction between gases, the volumes of the reacting gases and the volumes of any gaseous products are in the ratio of small whole numbers provided the volumes are measured at the same temperature and pressure.

Molar volume

22.4 L

24 L

Assumptions of the Kinetic theory of Gases

1. Gases are made up of particles that are in continuous motion, colliding with each other and with the walls of the container.
2. There are no attractive or repulsive forces between the molecules of a gas.
3. The volume of the gas molecules is negligible compared with the spaces between them.
4. When molecules collide, the collisions are perfectly elastic.
5. The average kinetic energy of the molecules is proportional to the temperature in Kelvin scale.

Limitations to the Kinetic theory of Gases

1. There are attractive and repulsive forces between the molecules of a gas.
2. The volume of the molecules is not negligible compared with the space that they occupy.
3. Collisions are not perfectly elastic.